What type of acid is sulfuric acid?
a. diprotic
b. triprotic
c. momoprotic
d. none
What is a. diprotic
100
Which compound can act as both a Bronsted-Lowry acid and a Bronsted-Lowry acid?
a. ammonia
b. sodium hydroxide
c. hydrochloric acid
d. water
What is d. water
100
What is the charge on the hydronium ion?
a. 2-
b. 2-
c. 1+
d. 0
What is c. 1+
100
What is pH?
a. positive log of the hydrogen ion concentration
b. negative log of the hydroxide ion concentration
c. negative log of the hydrogen ion concentration
d. positive log of the hydroxide ion concentration
What is c. negative log of the hydrogen ion concentration
100
Which type of solution is one with a pH of 8?
a. neutral
b. acidic
c. basic
d. depends on the solution
What is c. basic
200
What characterizes a strong acid or base?
a. ionic bonding
b. complete ionization in water
c. presence of a hydrogen or hydroxide ion
d. polar covalent bonding
What is b. complete ionization in water
200
With solutions of strong acids and strong bases, the word "strong" refers to:
a. solubility
b. degree of ionization
c. normality
d. molarity
What is b. degree of ionization
200
What is another name for the acid dissociation constant?
a. mole fraction
b. equilibrium constant
c. ionization constant
d. rate constant
What is c. ionization constant
200
A 0.12M solution of an acid that ionizes only slightly in solution would be termed:
a. dilute and weak
b. concentrated and weak
c. strong and dilute
d. concentrated and strong
What is a. dilute and weak
200
Which is a type of indicator?
a. bleach
b. alcohol
c. ammonia
d. phenolphthalein
What is d. phenolphthalein
300
Red litmus turns _____ in contact with ______.
a. red, base
b. both b and c
c. blue, base
d. pink, acid
What is c. blue, base
300
Neutralization reactions always produce
a. strong acid and weak base
b. water
c. salt and water
d. weak acid and strong base
What is c. salt and water
300
Which of the following usuallu makes a substance dissolve faster in a solvent?
a. agitating the solution
b. increasing the particle size of the solute
c. lowering the temperature
d. decreasing the number of particles
What is a. agitating the solution
300
Standard conditions when working with gases are defined as:
a. 0C and 101.3kPa
b. 0K and 101.3kPa
c. 0C and 1 kPa
d. 0K and 1 kPa
What is a. 0C and 101.3kPa
300
The pressure of a gas in a container is 152mmHg. This is equivalent to (given: 1atm=101.3kPa):
a. 0.3atm
b. 0.2atm
c. 0.4atm
d. 2 atm
What is b. 0.2atm
400
To increase the solubility of a gas at constant temperature from 1.20 g/L at 1.4 atm, to 2.3g/L, the pressure would have to be increased to: (given S1/P1 = S2/P2)
a. 1.37atm
b. 0.37atm
c. 0.7atm
d. 2.7atm
What is d. 2.7atm
400
What is the molarity of a solution containing 56 grams of solute in 959 mL of solution? Molar mass = 26 g/mol
Given: molarity = moles of solute / liters of solution
a. 2.1M
b. 0.0022M
c. 1.5M
d. 2.2M
What is d. 2.2M
400
How many mL of a 2.0M NaBr solution are needed to make 200.0mL of 0.50 NaBr? Given: M1V1 = M2V2
a. 25mL
b. 50mL
c. 100mL
d. 150mL
What is b. 50mL
400
If the density of an unknown gas "Z" is 4.50 g/L at STP, what is the molar mass of Z?
a. 0.201g/mol
b. 101 g/mol
c. 5.00 g/mol
d. 26.9g/mol
What is b. 101 g/mol
400
The products of the self-ionization of water are:
a. H3O+ and H2O
b. OH+ and H-
c. OH- and OH+
d. OH- and H+
What is d. OH- and H+
500
In a neutral solution, the [H+] is ______.
a. equal to [OH-]
b. 10^-14M
c. 1x10^7M
d. zero
What is a. equal to [OH-]
500
What is the pH and pOH of a 6.7 x10^-3M NaOH solution?
a. pH 16.17 pOH -2.17
b. pH 2.17 pOH 11.8
c. pH -2.17 pOH 16.17
d. pH 11.8 pOH 2.17
What is d. pH 11.8 pOH 2.17
500
What is the formula for phosphoric acid?
a. H3PO4
b. HPO2
c. HPO4
d. H2PO3
What is a. H3PO4
500
The formula of the hydrogen ion is often written as:
a. H+
b. OH+
c. H2O+
d. H4N+
What is a. H+
500
The reaction 2Fe + 3Cl2 -> 2FeCl3 is an example of which type of reaction?
a. single replacement
b. combustion
c. decomposition
d. combination